Fall 2019

CHEM 131 Final Exam Review Worksheet

Based on problems from the ACS Exam Review booklet, published ACS Chemistry Olympiad Exams, OpenStax Chemistry,
and other sources. Note: The final exam may cover topics not included on this list or in the practice problems.

Part I Part II Part IV

Introduction to Chemistry Gas Laws The Structure of the Atom
standard conditions (STP)
Scientific Method PV = nRT Energy
R = 0.082057 L.atm/mol.K E = hν = hc/λ
Measurements R = 8.3145 J/mol.K c = λν
significant figures h = 6.6260693 x 10-34 J.s
percent yield Enthalpy c = 2.99792458 x 108 m/s
percent error calorimetry
q = mcpΔT The Bohr Model
Atoms 1 1 1
isotopes Hess’s Law = Rh � 2 − 2 �
𝜆𝜆 𝑛𝑛𝑓𝑓 𝑛𝑛𝑖𝑖
atomic number standard conditions, ΔH°
mass number
1 1
symbol ΔHrxn = ΔH1 + ΔH2 + … ∆𝐸𝐸 = k � 2 − 2�
protons, neutrons, electrons 𝑛𝑛1 𝑛𝑛2
average atomic mass ΔH = ∑ΔHf products – ∑ΔHf reactants
from isotopes products − reactants Quantum Numbers
n: principal
Molecules ΔHbonds = ∑ΔHbroken – ∑ΔHformed ℓ: angular momentum
percent composition bonds broken – formed mℓ: magnetic
counting atoms/molecules ms: spin

Concentration Part III Electron Configuration

molarity atoms vs. ions
molality Intermolecular Forces
percent by mass (w/w)% Periodic Trends
dispersion
percent by mass-volume (w/v)% Zeff: effective nuclear charge
dipole-dipole
percent by volume (v/v)% atomic size
hydrogen bonds
ionic size
donors vs. acceptors
Chemical Reactions electronegativity
induced-dipole
balancing electron affinity
like-dissolves-like
listing coefficients
summing coefficients Bonding Models
Colligative Properties
classification Lewis structures
vapor pressure lowering
valence electrons
∆Psolvent = Xsolute P°solvent
Stoichiometry resonance structures
Psolvent = Xsolvent P°solvent
g → mol → percent yield boiling point elevation
formal charges
molarity → mol → percent yield ∆Tb = 𝒾𝒾Kbm
VSEPR and geometry
actual vs. percent yield polarity
freezing point depression Valence Bond Theory
titrations
∆Tf = 𝒾𝒾Kfm hybrid atomic orbitals
osmotic pressure multiple bonds (π and σ)
∏ = 𝒾𝒾MRT bond angles

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Part I

1. What is the correct reading of the buret shown?

(A) 30.20 mL (B) 30.25 mL

(C) 30.30 mL (D) 31.75 mL

2. Which of the following is the best name for TiO2?

(A) titanium oxide (B) titanium dioxide
(C) titanium(IV) dioxide (D) titanium(IV) oxide

3. Which of the following is the formula for barium phosphate?

(A) BaPO4 (B) Ba3PO4
(C) Ba3(PO4)2 (D) Ba(PO4)3

4. Which of the following is the best name for Mo3N2?

(A) molybdenum(II) nitrite (B) molybdenum(III) nitride
(C) molybdenum nitride (D) molybdenum(II) nitride

5. Which of the following is the best name for MnS2?

(A) magnesium sulfide (B) manganese (IV) sulfide
(C) manganese disulfide (D) magnesium(IV) sulfide

6. Europium has two stable isotopes, 151Eu and 153Eu. 151Eu has a mass of
150.9199 amu and 153Eu has a mass of 152.9212 amu. What are the
abundances of 151Eu and 153Eu?
151Eu 153Eu

(A) 32.75% 67.25%

(B) 47.81% 52.19%
(C) 75.31% 24.69%
(D) 39.92% 60.08%

7. Which of the following is the correct symbol for an ion containing 30

neutrons, 18 electrons, and an overall charge of +6?
(A) 54
24Cr
6+
(B) 60
30Zn
6+
(C) 48
18Ar
6+
(D) 78
48Nd
6+

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8. What is the concentration of chloride ions in a solution formed by mixing

150.0 mL of 1.50 M NaCl with 250.0 mL if 0.750 M MgCl2?
(A) 0.563 M (B) 1.03 M (C) 1.50 M (D) 2.25 M

9. In which of the following substances is chlorine in the lowest oxidation state?

(A) Cl2 (B) KCl (C) KClO (D) KClO4

10. The formula for terbium phosphate is TbPO4. What is the formula for terbium
sulfate?
(A) Tb2SO4 (B) TbSO4 (C) Tb2(SO4)3 (D) Tb(SO4)2

11. A mixture is prepared by adding 50.0 mL of 0.200 M NaOH to 75.0 mL of

0.100 M NaOH. What is the [OH−] in the mixture?
(A) 0.0600 M (B) 0.0800 M
(C) 0.140 M (D) 0.233 M

12. A compound with 69.41% C, 4.16% H, and 26.42% O has a molar mass of
230-250 g/mol. What is its molecular formula?
(A) C13H9O4 (B) C14H10O4
(C) C13H6O4 (D) C15H14O3

13. What is the coefficient for oxygen gas when the reaction for the combustion of
propane, C3H8, is balanced?
(A) 1 (B) 3 (C) 5 (D) 9

14. Boron carbide, B4C, is made by the high temperature reaction of boron oxide
with graphite, yielding carbon monoxide as a by-product.
__ B2O3 + __ C → __ B4C + __ CO
What is the sum of the smallest whole number coefficients for reactants and
products in the balanced equation?
(A) 9 (B) 10 (C) 15 (D) 16

15. What is the sum of the smallest whole number coefficients used to balance the
following reaction?
___ CaCl2(aq) + ___ K3PO4(aq) → ___ Ca3(PO4)2(s) + ___ KCl(aq)

(A) 1, 1, 3, 6 (B) 3, 2, 1, 6 (C) 3, 3, 2, 6 (D) 3, 2, 1, 3

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16. What is the oxidation number of technetium in NaTcO4?

(A) +2 (B) +4 (C) +7 (D) +8

17. What is the oxidation number for carbon in methanol, CH3OH?

(A) −2 (B) +2 (C) +4 (D) −4

Classify the following reactions by using the labels given below.

(A) synthesis
(B) decomposition
(C) double displacement
(D) single replacement
(E) combustion

18. 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(g)

19. Sodium hydroxide is mixed with hydrochloric acid.
20. P4(s) + 10 Cl2(g) → 4 PCl5(ℓ)
21. Lead nitrate reacts with potassium sulfate in aqueous solution.
22. Zn(NO3)2(aq) + Cu(s) → Zn(s) + Cu(NO3)2(aq)
23. Ag2CO3(aq) → Ag(s) + CO2(g) + O2(g)

24. Aluminum reacts with sulfur to form aluminum sulfide. If 27.00 g of Al react
with 95.70 g of Te, what is the theoretical yield of aluminum telluride in
grams?
(A) 109.2 g (B) 218.5 g (C) 70.6 g (D) 38.6 g

25. In a combustion reaction, benzene, C6H6, reacts with oxygen gas to form CO2 and
H2O. How much oxygen gas is required for the complete combustion of 1.0 mol
C6H6?
(A) 6.0 mol (B) 7.5 mol (C) 9.0 mol (D) 12 mol

26. Barium chloride reacts with sodium sulfate according to the following equation:
BaCl2(aq) + Na2SO4(aq) → BaSO4(s) + 2 NaCl(aq)
A student mixes a solution containing 10.0 g BaCl2 with a solution containing
10.0 g Na2SO4 and obtains 12.0 g BaSO4. What is the percent yield for this
reaction?
(A) 60.0% (B) 73.1% (C) 93.3%
(D) The isolated product is most likely wet, since the yield would otherwise be
greater than 100%.

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27. Which of the following graphs would best represent the changes when 0.10 M
barium hydroxide is titrated with 0.10 M sulfuric acid?

(D)

28. In order to determine the concentration of a sodium hydroxide solution,

titrations were performed with a standardized 0.200 M HCl solution.
Phenolphthalein was used as the indicator.
Trial Vol HCl Vol NaOH [NaOH] calculated
1 21.43 19.26 0.223
2 18.57 16.73 0.222
3 22.20 21.14 0.210

Which explanation best accounts for the lower calculated concentration for
NaOH in Trial 3?
(A) Some of the neutralized solution from Trial 2 was left in the flask for Trial
3.
(B) The number of drops of phenolphthalein was doubled in Trial 3.
(C) 0.250 M for [HCl] was accidentally used in the [NaOH] calculation.
(D) A few drops of NaOH spilled on the benchtop during Trial 3.

29. What mass of NaHCO3 (84.0 g/mol) is required to completely neutralize 25.0
mL of 0.125 M H2SO4?
(A) 0.131 g (B) 0.262 g (C) 0.525 g (D) 1.05 g

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Part II

30. A sample of 54.0 g of methanol, CH3OH, is heated from 25.0 °C to 35.0 °C.
How much heat is required? The specific heat capacity for methanol is 2.48 J
g-1 K-1.
(A) 0.0049 J (B) 0.0747 J (C) 1340 J (D) 4690 J

31. A sample of NaOH(s) was added to water in a constant pressure calorimeter.

The temperature was monitored as the NaOH dissolved. The data are given
below. Determine the heat released during the solution process. The specific
heat for the solution is 4.18 J g−1 .°C−1.
Mass of H2O 100.00 g
Mass of NaOH(s) 10.00 g
Initial temperature of water 24.0 °C
Final temperature of solution 48.2 °C

(A) 1.01 x 103 J (B) 2.66 x 103 J

(C) 1.01 x 104 J (D) 1.11 x 104 J

32. For the reaction:

3 H2(g)+ N2(g) → 2 NH3(g) ΔH° = −97 kJ/mol
The H2 and N2 bond energies are 436 and 941 kJ/mol, respectively. What is the
bond energy for a single N−H bond in kJ/mol?
(A) 246 (B) 359 (C) 391 (D) 782

33. Given the standard enthalpy changes for the reactions below, calculate the
standard enthalpy change for the reaction:
P4O6(s) + 2 O2(g) → P4O10(s)
P4(s) + 3 O2(g) → P4O6(s) ΔH° = −1640 kJ/mol
P4(s) + 5 O2(g) → P4O10(s) ΔH° = −2940 kJ/mol

(A) −4.58 x 103 kJ (B) −1.30 x 103 kJ

(C) 1.79 kJ (D) 4.82 x 106 kJ

34. Choose the reaction(s) for which the heat of formation is equal to the heat of
reaction.
I. ½ N2(g) + O2(g) → NO2(g) ΔH° > 0
II. SO2(g) + ½ O2(g) → SO3(g) ΔH° < 0

(A) I only (B) II only

(C) Both I and II (D) Neither I nor II

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35. The combustion of 2-propanol (M = 60.0 g/mol) occurs according to the

reaction:
2 CH3CHOHCH3(ℓ) + 9 O2(g) → 6 CO2(g) + 8 H2O(ℓ)
CH3CHOHCH3(ℓ) CO2(g) H2O(ℓ)
∆𝐻𝐻𝑓𝑓° (kJ/mol) −318.2 −393.5 −285.8

What is q for the combustion of 15.0 g of 2-propanol?

(A) −5.01 x 102 kJ (B) −1.00 x 103 kJ
(C) −2.01 x 103 kJ (D) −4.01 x 103 kJ

36. What is ΔH° for the reaction shown?

2 H2S(g) + 3 O2(g) → 2 H2O(ℓ) + 2 SO2(g)

∆𝐻𝐻𝑓𝑓° for H2S(g) = −20.15 kJ/mol

∆𝐻𝐻𝑓𝑓° for H2O(ℓ) = −285.8 kJ/mol
∆𝐻𝐻𝑓𝑓° for SO2 (g) = −296.4 kJ/mol

(A) −19.4 kJ/mol (B) −347.7 kJ/mol

(C) −562.1 kJ/mol (D) −1124.1 kJ/mol

37. A sample of neon gas is held at 25.0 °C and 1.0 atm in a cylinder with a
movable piston. Under these conditions, the gas occupies 5.0 L. What volume
does the gas occupy at 12.5 °C and 1.0 atm?
(A) 2.5 L (B) 4.8 L (C) 5.2 L (D) 10 L

38. Which of the following is/are true for gases?

1. The amount of a gas in moles in inversely proportional to its volume at
constant temperature and pressure.
2. The pressure of a gas is inversely proportional to its temperature at constant
volume and amount in moles.
3. The volume of a gas is directly proportional to its temperature at constant
pressure and amount in moles.

(A) 1 only (B) 2 only

(C) 3 only (D) 1 and 3 (E) 2 and 3

39. Under what conditions does the behavior of real gases deviate most from that
predicted by the ideal gas law?
(A) low P, low T (B) high P, low T
(C) low P, high T (D) high P, high T

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40. A gas with P = 615 mmHg is contained in the U-tube as shown. If h = 65 mm,
what is the atmospheric pressure?

(A) 550 mmHg (B) 615 mmHg

(C) 680 mmHg (D) 760 mmHg

41. What volume would a 16.0 g sample of oxygen gas occupy at standard
temperature and pressure?
(A) 5.60 L (B) 11.2 L (C) 12.2 L (D) 24.4 L

42. Into both ends of a meter-long glass tube, samples of gas are introduced
simultaneously. One end receives HCl gas while the other end receives NH3
gas. When the gases meet in the tube, a reaction occurs and solid ammonium
chloride forms. Where in the tube does NH4Cl(s) form?
(A) At the center of the tube.
(B) Closer to the end where the HCl was introduced.
(C) Closer to the end where the NH3 was introduced.
(D) Uniformly in all positions in the tube.

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Part III

43. Which statement concerning the phase diagram is incorrect?

(A) Only solid exists at point #1.

(B) At point #3, all three phases (solid, liquid, and gas) are in equilibrium.
(C) Solid and liquid are in equilibrium at point #4.
(D) At point #5, only gas is present.

44. The lattice energy of MgO is much larger than that of LiF. What contributes
most to this difference?
(A) Mg2+ is a smaller ion than Li+, and O2- is a smaller ion than F-.
(B) F is more electronegative than O, and Li is more electropositive than Mg.
(C) MgO contains doubly charged ions, while LiF contains singly charged
ions.
(D) MgO contains more electrons than LiF.

45. Pure samples of which of the following exhibit hydrogen bonding?

I. CH3OH II. CH3NO2 III. CH3CN
(A) I only (B) I and II only
(C) II and III only (D) I, II, and III

46. Which physical property decreases with an increase in intermolecular forces?

(A) boiling point (B) vapor pressure
(C) enthalpy of vaporization (D) viscosity

47. Which molecule has a dipole moment of zero?

(A) CO (B) CO2 (C) CH2O (D) CH3OH

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48. Which of the following compounds would have the highest vapor pressure?
(A) CH3CH2CH3 (B) CH3CH2CH2OH
(C) CH3OOCH3 (D) CH3CH2COOH

49. What is the principal energetic factor in the lack of miscibility between C6H14(ℓ)
and H2O(ℓ)?
(A) The strength of intermolecular forces of attraction between C6H14(ℓ)
molecules
(B) The strength of intermolecular forces of attraction between H2O(ℓ)
molecules
(C) The difference between the molecular weights of the molecules
(D) The difference in electronegativity between carbon and hydrogen

50. The value of which concentration unit for a solution changes with temperature?
(A) molarity (B) molality
(C) mole fraction (D) mass percentage

51. A student wishes to determine the molar mass of a pure solid organic compound.
Which measurement would be most useful?

(A) melting point of the solid

(B) heat of combustion of the solid
(C) freezing point depression of the solid dissolved in pure benzene
(D) solubility in pure benzene

52. Which aqueous solution exhibits the largest freezing point depression?
(A) 1.0 m KBr (B) 0.75 m C6H12O6
(C) 0.5 m MgCl2 (D) 0.25 m Ga2(SO4)3

53. How would the freezing point depression of a 0.05 m CaCl2 solution compare
with that of an NaCl solution? The freezing point depression would be:

(A) less than that for 0.10 m NaCl solution.

(B) between that for a 0.10 m NaCl and a 0.20 m NaCl solution.
(C) between that for a 0.20 m NaCl and a 0.30 m NaCl solution.
(D) greater than that of a 0.30 m NaCl solution.

54. Interferon is a water-soluble protein. A solution prepared by dissolving 15.0 mg

of interferon in 2.50 mL of H2O exhibits an osmotic pressure of 5.80 mmHg at
25 °C. What is the molar mass of interferon?
(A) 1.92 x 104 g/mol (B) 1.92 x 107 g/mol
(C) 1.95 x 106 g/mol (D) 1.61 x 103 g/mol

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Part IV

55. The wavelength of one of the spectral lines of helium is 492 nm. What is
the energy of a photon at this wavelength?
(A) 3.26 x 10−40 J (B) 3.26 x 10−31 J
(C) 4.04 x 10−28 J (D) 4.04 x 10−19 J

56. Which of the following statements is incorrect?

(A) It is not possible to know the exact location and energy of an

electron at the same time.
(B) Electrons have both wave-like and particle-like properties.
(C) The behavior of electrons around an atom can be described by
circular orbits around the nucleus.
(D) Quantum numbers define the orbitals available to an electron.

57. In the ground-state phosphorus atom, how many electrons have the
quantum numbers n = 3, ℓ = 1, and mℓ = −1?
(A) 0 (B) 1 (C) 2 (D) 3

58. For a hydrogen atom, which change in principal quantum number would
correspond to emission of a photon with the longest wavelength?
(A) n = 4 → n = 1 (B) n = 5 → n = 2
(C) n = 1 → n = 5 (D) n = 2 → n = 4

59. Which of the following gas phase ions has the largest number of
unpaired electrons in its ground state?
(A) Cr3+ (B) Co3+ (C) Ni2+ (D) Cu2+

60. A sulfur atom in its ground state has the electron configuration:
1s2 2s2 2p6 3s2 3p4
How many orbitals are occupied by at least one electron?
(A) 3 (B) 5 (C) 8 (D) 9

61. Rank the elements Si, P, Ar, and Na in order of increasing atomic size.
(A) Na < P < Si < Ar (B) Ar < P < Si < Na
(C) Na < Si < P < Ar (D) Ar < Si < P < Na

62. Of the atoms listed, which has the largest third ionization energy?
(A) Ca (B) Al (C) Mg (D) Si

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63. Consider the Lewis structure below. What are the formal charges on the
atoms?

N C O
(A) −1 0 0
(B) −1 +1 −1
(C) 0 0 −1
(D) −1 −1 +1

64. Arrange the following species in order of decreasing C−O bond length.
CO32− CO CO2
2−
(A) CO3 , CO, CO2 (B) CO2, CO, CO32−
(C) CO, CO32−, CO2 (D) CO32−, CO2, CO

65. What is the formal charge on the oxygen atom in carbon monoxide?
(A) 0 (B) +1 (C) −1 (D) −2

66. The structure of vinylamine is shown below. What geometry is exhibited

by each of the marked atoms?

Geometry at X Geometry at Y
(A) trigonal planar trigonal planar
(B) trigonal planar trigonal pyramidal
(C) trigonal pyramidal trigonal planar
(D) trigonal pyramidal trigonal pyramidal

67. How many σ and π bonds are in 1,3-butadiene, CH2=CH−CH=CH2?

(A) 7 σ and 2 π (B) 2 σ and 7 π
(C) 9 σ and 2 π (D) 2 σ and 9 π

68. What is the geometry of SF4?

(A) tetrahedral (B) see-saw

(C) square planar (D) trigonal pyramidal

69. For the two species listed, which have the same shape?

(A) CO2 and SO2 (B) CCl4 and SiCl4

(C) C2H6 and B2H6 (D) NO3- and PO33-

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70. How many σ bonds are present in the molecule below?

H O

H C C
C C OH

C C
H C H

(A) 4 (B) 10 (C) 14 (D) 15 (E) 19

Determine the hybridization of each atom marked in the molecule below.

(A) sp (B) sp2 (C) sp3 (D) sp3d (E) sp3d2

_____ 71. atom #1

_____ 72. atom #2

_____ 73. atom #3

_____ 74. atom #4

Determine the geometry of each atom marked in the molecules below.

(A) linear (B) bent (C) trigonal pyramidal (D) trigonal planar (E) tetrahedral

_____ 75. atom #5

_____ 76. atom #6

_____ 77. atom #7

78. Of the three molecules shown (for Problems #75-77), which will form hydrogen bonds?

(A) The molecule with the carbon marked #5.

(B) The molecule with the nitrogen marked #6.
(C) The molecule with the carbon marked #7.
(D) Impossible to tell without further information.

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